JEOPARDY!

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Click Once to BeginJEOPARDY!Chemistry Final Review


JEOPARDY!

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The Periodic Table

Atoms and Ions

Ionization Energy

Electron Configuration

Electron Affinity

Miscellaneous


Which of the following is a metalloid?

H, Ge, S, Kr or Ag


Ge


How did Dmitri Mendeleev organize the elements in

his creation of the periodic table?


By their atomic mass


What group number are the Chalcogens?


Group number 16


What are the two group names of the elements found

in the two rows under the periodic table?


The top row is called Lanthanide series and the bottom row is called Actinide series


What is the relationship between effective nuclear

charge and valance electrons going down a column and

across a row?


Going down a column, the effective nuclear charge experienced by valance electrons changes far less that it does

across a row


How are ions formed?


Ions are formed when electrons are gained or

lost.


What is the difference between a cation and an

anion?


A cation is a positive ion whereas an anion is a

negative ion


What are the trends in atomic radii with each column in the

periodic table?


Atomic radius increases from top to bottom within

each column.


Arrange the following in order of increasing atomic

radius...Na, Be, Mg


Na, Mg, Be


Why does atomic radius decrease from left to right within each row of the periodic

table?


The increase in effective nuclear charge as one moves across the row steadily draws the valence electrons

closer to the nucleus, causing the atomic radius to decrease.


What is ionization energy?


The minimum energy required to remove an

electron from the ground state of the isolated gaseous atom or ion


Which show a lower ionization energy, the alkali metals or the noble gases?


The alkali metals.


Arrange the noble gases in increasing ionization energy

order


He, Ne, Ar, Kr and Xe.


Which has a greater ionization energy: an s- and p-block

element or a transition-metal element?

Daily Double!!!


The s- and p-block elements


Which will have the greater ionization energy, Ca or S?


S


As an atomic number increases the number of _____ also increases.


Electrons or protons.


What are valance electrons?


An electron in the outer shell of an atom.


Which element’s electron configuration ends with 4p3?


As


What is the electron configuration of Xe using noble gas notation?


[Kr]4d105s25p6


Write the electron configuration for the following

ions:1. Ga3+

2. Cr3+


1. [Ar]3d10

2. [Ar]3d3


Explain electron affinity


The energy change that occurs when an electron is added to a gaseous atom is called the electron affinity because it measures the

attraction, or affinity, of the atom for the added electron.


When an electron is added what happens to the atoms?


Energy is released when an electron is

added.


Which group has the most negative electron affinities?


The Halogens.


Why do the noble gases have a highly positive electron affinity?

Daily Double!!!


The Noble Gases already have a full

outer shell and therefore occupying a

higher-energy sub-shell is

energetically very unfavorable

making their electron affinities very

positive


How do electron affinities change moving down a group?


They don’t change! Not very much

anyways..


What are the properties of metals?


Shiny luster, conduct heat and electricity and are malleable

and ductile


What is an ionic substance?


A compound of metals with nonmetals.


As atomic number increases what happens to the

melting and boiling points of the halogens?


Since they are all typically nonmetals, their melting and boiling points increase with increasing atomic number.


Write the electron configuration for Ca and

Ca2+


Ca: [Ar]4s2

Ca2+: [Ar]


Why is O2- larger than O?


O2- is larger than O because increased repulsions that accompany addition of electrons

cause the electron cloud to expand


Final Jeopardy


Click Once to Begin

Using the figure below predict which will be greater, the P---Br bond length in PBr3 or the

As---Cl bond length in AsCl3


Click for answer!!Answer: P---Br

JEOPARDY!

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